A solution contains 0.0330 M Pb2+(aq) and 0.0330 M Sr2+(aq). If you add SO42−(aq), what will be the concentration of Pb2+(aq) when SrSO4(s) begins to precipitate?

A technician would like to standardize an unknown Ca(OH)2 solution. It takes 18.53 mL of a 0.174 M solution of HCI to titrate 25.00 mL the unknown Ca(OH)2 solution. Calculate the molarity of the Ca(OH)2 solution. Tip: Don't forget to consider the mole ratio between HCl and Ca(OH)2. 2 HCI (aq) + Ca(OH), (aq) CaCl2 (aq) + 2 H2O (1)

A solution of hydrogen peroxide was titrated with a solution of potassium permanganate (see reaction).5 H 2O 2(aq) + 2 KMnO 4(aq) + 3 H 2SO 4 -> 5 O 2(g) + 2 MnSO 4(aq) + K 2SO 4(aq) + 8 H 2O(l)It required 75.00 mL of 0.1456 M KMnO 4 to titrate 2.623 g of the solution containing hydrogen peroxide. What was the mass percentage of H 2O 2 in the solution?

A scientist is investigating the solubility of two polyatomic ions, oxalate (C2O2−4C2⁢O42−) and arsenate (AsO3−4AsO43−), which are not listed in the table of solubility guidelines. The scientist starts with four solutions made of water-soluble salts. Solution A contains sodium arsenate. Solution B contains ammonium oxalate. Soution C contains silver chlorate. Solution D contains aluminum bromide. Solution Solute Color of Solution A Na3AsO4Na3⁢AsO4 colorless B (NH4)2C2O4(NH4)2⁢C2⁢O4 colorless C AgClO3AgClO3 colorless D AlBr3AlBr3 yellow The results of mixing each solution in pairs are shown in the table. Experiment Solutions Mixed Result 1 A + B no precipitate, colorless solution 2 A + C brown precipitate 3 A + D white precipitate 4 B + C white precipitate 5 B + D white precipitate 6 C + D yellow precipitate Identify the formula for each precipitate that forms. precipitate from A+C:   precipitate from A+D:   precipitate…

You have been provided with a 2.08 x 10-2 L  sample of lithium hydroxide (LiOH) of unknown concentration. You perform a titration with 2.19 M nitric acid (HNO3), and find that 24.6 mL are required to reach the equivalence point (as determined using a coloured indicator). What is the concentration of the lithium hydroxide solution in mol L-1?

A chemist needs to determine the concentration of a solution of nitric acid, HNO3. She puts 905 mL of the acid in a flask along with a few drops of indicator. She then slowly adds 0.200 mol L Ba(OH)2 to the flask until the solution turns pink, indicating the equivalence point of the titration. She notes that 225 mL of Ba(OH)2 was needed to reach the equivalence point. Solution map In this titration, the concentration of base is known and can be used to calculate the unknown acid concentration: concentration of base → moles of base → moles of acid → concentration of acid Part A How many moles of Ba(OH)2 are present in 225 mL of 0.200 mol L-1 Ba(OH)2? Express your answer numerically in moles. • View Available Hint(s) Vo AEO ? mol Ba(OH)2 Submit

You have a 1.153 g sample of an unknown solid acid, HA, dissolved in enough water to make 20.00 mL of solution. HA reacts with KOH(aq) according to the following balanced chemical equation:HA(aq)+KOH(aq) --------->KA(aq)+H2O(l)       If 14.90 mL of 0.585 M KOH is required to titrate the unknown acid to the equivalence point, what is the concentration of the unknown acid? ______ M      What is the molar mass of HA? _____  g/mol

Normal calcium levels in the blood should be between 9.0 and 10.5 mg/dL. Calcium levels in the blood can be determined by adding oxalate ion to precipitate calcium oxalate, CaC2O4, followed by dissolving the precipitate in aqueous acid and titrating the resulting oxalic acid (H2C2O4) with KMnO4. 5 H2C2O4 (aq) + 2 MnO4–(aq) + 6 H+(aq) yields 10 CO2 (g) + 2 Mn2+(aq) + 8 H2O(l) What is the concentration of Ca2+ (mg/dL) in a 10.0 mL sample of blood if 10.54 mL of 9.88 x 10–4 M KMnO4 solution is needed for the titration.

concd upon the addition of 15.1 mL of 0.611 M aqueous calcium hydroxide solution. What is the concentration (in M) of the HI solution? Tesaration analysis of a 24.0 mL agueous HI solution was performed and the endpoint was HI(aq) + Ca(OH)2 (aq) > Cal (aq) + H2O(1) A: 0.769

50 mL of a 1.067 M solution of HCI was diluted to 250 mL. The diluted HCI solution was then titrated with an unknown concentration of KOH. It is found that an average volume of 24.20 mL of KOH is required to reach an endpoint in a titration with 25.00 mL of the dilute acid solution. The equation for the reaction is; H(aq) + OH(aq) →→> H₂O (1) The concentration of KOH is 0.2205 M Calculate the concentration of the KOH in g/L (you will need to find the formula weight of KOH to do this) 15| ΑΣΦ ? g/L